Detailed chemical kinetic models are important to the understanding and prediction of combustion properties. Better estimations require an accurate description of thermochemistry and kinetic rate parameters. This study identifies important reaction pathways at the low temperature chemistry of branched conventional and alternative fuels. Rate constants and branching ratios for important reactions are provided and important phenomena are investigated. The thermochemistry and kinetics of the 2-methylhexane model, an important component in gasoline surrogate, is updated using recent group values and rate rules from the literature. New reactions, such as hydroperoxyalkylperoxy (OOQOOH) alternative isomerization, are also added to the model. The results show that both conventional and alternative isomerization of OOQOOH radicals significantly affect the model reactivity. The kinetics of a biofuel; iso-butanol, is also investigated in this study to understand alcohol combustion chemistry and identify sensitive reactions that require more attention. The results indicate that iso-butanol is sensitive to the chain propagation reaction of α-RO2 radical and the water elimination of γ-QOOH. Because both reactions decrease model reactivity, accurate rate constants are needed to correctly determine fuel reactivity. In light of the above mentioned kinetic modeling studies, high levels computational chemistry calculations were performed to provide site-specific rates rules for OOQOOH conventional isomerization considering all possible reaction sites. This is also one of the first studies to investigate the effect of chirality on calculated rate constants. Results indicate that chirality is important when two chiral centers exist in the reactant. OOQOOH alternative isomerization rate constants are usually assigned in analogy to the isomerization of an alkylperoxy (RO2) radical which may introduce some uncertainty. To test the validity of using analogous rates, this study calculates the rate constants for selected alternative isomerization reactions. The effect of intramolecular hydrogen bonding in the calculated energies and rate constants for different reaction pathways is investigated. The result shows that alternative isomerization is a competing pathway only when it proceeds via a less strained transition state relative to the conventional isomerization transition state. A detailed analysis of the hydrogen bonding effect helped to identify cases where assigning rates in analogy may not be valid.

Increasingly stringent legislations call for more efficient and cleaner combustion technology as well as sustainable fuels. Chemical kinetic models are required in designing and optimizing novel engine concepts as well as selecting appropriate renewable fuels. Among the many reactions controlling fuel reactivity, OH + Fuel elementary reaction is one of the most important reactions that plays a critical role from low to high temperatures. In this thesis, OH + Fuel elementary reactions are studied for a wide spectrum of conventional and renewable fuels. The overall rate coefficients are measured in a shock tube using OH time-history profiles recorded with a UV laser diagnostic. Alkanes constitute important components of gasoline and diesel. Overall rate coefficients are measured for a series of large branched alkanes and the rate rules are derived based on the next-nearest-neighbor classification method. The strength of this method lies in the ability to predict the rate coefficients for large and/or highly-branched alkanes, where both experiments and theoretical calculations are hard to reach. Next, OH reactions with bio-derived fuels, methanol and cyclic-ketones, are studied. For OH + methanol reaction, site-specific contributions from different C-H bonds are quantified using deuterium kinetic isotopic effect, and the measured rate coefficients are found to improve the general behavior of a detailed methanol kinetic model. Reactions of cyclic ketones with OH radicals are found to exhibit similar reactivity as those of similar carbon length acyclic ketones + OH reactions. Acetaldehyde is one of the most abundant hazardous byproducts in the combustion of various fuels. Similar to methanol, OH + acetaldehyde reaction is 4 studied at the site-specific level and the importance of competing reaction channels are quantified at high temperatures. Finally, reactions of OH + cyclohexadienes and OH + trimethylbenzenes, relevant for the fate of polycyclic aromatics hydrocarbons, are investigated. A highly complex temperature dependence is observed for these molecules, a six-parameter Arrhenius expression is needed to describe the overall reactivity. The work reported in this thesis provides elementary reaction data that are highly valuable for increasing the fidelity and accuracy of predictive chemical kinetic models.

La combustion du noir de carbone (NC) dans le creuset d'une thermobalance est contrôlée à la fois par la réaction et par le transport de l'oxygène jusqu'à la surface du lit et à l'intérieur du lit poreux de NC.Les expériences menées en modifiant la masse de NC ont montré que la concentration en oxygène peut tomber à zéro avant d'atteindre le fond du lit. Ainsi, à un instant donné, seule une partie du lit est en combustion. Cette masse, appelée masse critique (mc) dépend de la température. Elle passe de 35 mg à 570°C à 17,5 mg à 650°C.Un gradient d'oxygène s'établi donc dans le lit. La modélisation du transport interne de l'oxygène a montré que la diffusion de Fick constitue une bonne approximation pour représenter ce transport.Des conseils pour extraire correctement une constante cinétique à partir d'expériences thermogravimétrique sont donnés. La procédure est adaptée en fonction de la précision souhaitée.Ainsi, l'utilisation de faibles masses afin de réduire au mieux l'effet de la masse et l'exothermicité de la réaction est fortement conseillée. L'influence de la diffusion externe du gaz peut être réduite en utilisant des creusets de très faibles hauteurs, ou en mettant l'échantillon le plus proche de la bouche du creuset en remplissant le fond du creuset avec un matériau inerte. / Combustion of carbon black (CB) in the crucible of a thermobalance is controlled by both carbon reactivity and oxygen transport from the oxidizing flux to the surface of the bed and within the porous bed.The experiments conducted by changing the mass of CB showed that the oxygen concentration can fall to zero before the bottom of the bed. Thus, at a given time, only a part of the bed is burning. This mass, called critical mass (mc), depends to temperature. It went from 35 mg at 570°C to 17.5 mg at 650°C.An oxygen gradient is thus established in the bed. The Modelling of the internal transport of oxygen showed that the Fick diffusion is a good approximation to represent the transport.Advices to correctly extract a kinetic constant using thermogravimetric experiments are given. The procedure is adjusted depending to the precision desired.Thus, the use of low masses to best reduce the mass and exothermic reaction effects is strongly recommended. The influence of stagnant gas can be reduced by using crucibles with very low height, or by placing the sample closest to the mouth of the crucible by filling the bottom of the crucible with an inert material.

This thesis describes the measurement of rate constants for gas phase reactions as a function of temperature (285 ≤ T/K ≤ 850) and pressure (48 ≤ P/Torr ≤ 700). One or both reactants was monitored directly in real time, using time–resolved resonance fluorescence (for atoms) and u.v. absorption (for radicals). Reactants were produced by exciplex laser flash photolysis. The technique was used to measure rate constants to high precision for the following reactions under the stated conditions: • H+O2+He->HO2+He and H+O2−→OH+O, for 800 ≤ T/K ≤ 850 and 100 ≤ P/Torr ≤ 259. A time–resolved study was performed at conditions close to criticality in the H2–O2 system. The competition between the two reactions affected the behaviour of the system after photolysis, and the rate constants were inferred from this behaviour. • H+C2H4+He<-->C2H5+He (T = 800 K, 97 ≤ P/Torr ≤ 600). The reactions were well into the fall–off region at all conditions studied. At 800 K, the system was studied under equilibrating conditions. The study provided values of the forward and reverse rate constants at high temperatures and enabled a test of a new theory of reversible unimolecular reactions. The controversial standard enthalpy of formation of ethyl, DH0f,298 (C2H5), was determined to be 120.2±0.8 kJ mol−1. Master Equation calculations showed that reversible and irreversible treatments of an equilibrating system should yield the same value for both thermal rate constants. • H+C3H5+He->C3H6+He (T = 291 K, 98 ≤ P/Torr ≤ 600) and O+C3H5 −→ products (286 ≤ T/K ≤ 500, 48 ≤ P/Torr ≤ 348). Both reactions were pressure–independent, and the latter was also independent of temperature with a value of (2.0±0.2) ×10−10 cm3 molecule−1 s−1. • H+C2H2+He<-->C2H3+He (298 ≤ T/K ≤ 845, 50 ≤ P/Torr ≤ 600). At 845 K, both reactions were in the fall–off region; rate constants were used to determine the standard enthalpy of formation of vinyl, ¢H0f,298 (C2H3), as 293±7 kJ mol−1. The value of this quantity has until recently been very controversial. • H+CH4 <--> CH3+H2. The standard enthalpy of formation of methyl, DH0 f,298 (CH3), was determined by re–analysing existing kinetic data at T = 825 K and 875 K. A value of 144.7±1.1 kJ mol−1 was determined. Preliminary models were examined to describe the loss of reactants from the observation region by diffusion and pump–out. Such models, including diffusion and drift, should prove useful in describing the loss of reactive species in many slow–flow systems, enabling more accurate rate constants to be determined.